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2. Calculate AH AG and AS for the following reaction given thermodynamic data below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values. HNO(g) + NH₂(g) → NH,NO,(s) Nitrogen NH, (9) NH, (84). HNO, (aq) HNO, (1) HNO, (9) NH.NO: (s) NH.NO: (aq) AH, (kJ/mol) AG", (kJ/mol) S (J/mol K) -16.5 192.5 -27.0 111.0 -111.3 146.4 -80.7 155.6 -74.7 266.4 -183.9 151.1 -190.6 259.8 ΔΗ. AG AS -46.1 -80.0 -207.4 -174.1 -135.1 -365.6 -339.9 3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)? Explain. 4. Based on the signs of AH and AS in which of the 4 categories does this reaction belong: spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high temperature or spontaneous at low temperature? 5. Use the AH and AS, calculated in question 2 as well as the equation below to calculate AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results compare to the answers in questions 2 and 4? Be careful with the units, AS, was calculated in units of J/(mol"K) while AH was calculated in kl/mol. AG AG AG @ 298K @ 10K 10,000K Activate V Go to Setting

2. Calculate AH AG and AS for the following reaction given thermodynamic data below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values. HNO(g) + NH₂(g) → NH,NO,(s) Nitrogen NH, (9) NH, (84). HNO, (aq) HNO, (1) HNO, (9) NH.NO: (s) NH.NO: (aq) AH, (kJ/mol) AG", (kJ/mol) S (J/mol K) -16.5 192.5 -27.0 111.0 -111.3 146.4 -80.7 155.6 -74.7 266.4 -183.9 151.1 -190.6 259.8 ΔΗ. AG AS -46.1 -80.0 -207.4 -174.1 -135.1 -365.6 -339.9 3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)? Explain. 4. Based on the signs of AH and AS in which of the 4 categories does this reaction belong: spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high temperature or spontaneous at low temperature? 5. Use the AH and AS, calculated in question 2 as well as the equation below to calculate AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results compare to the answers in questions 2 and 4? Be careful with the units, AS, was calculated in units of J/(mol"K) while AH was calculated in kl/mol. AG AG AG @ 298K @ 10K 10,000K Activate V Go to Setting

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Predict t for the following reaction. Is entropy increasing or decreasing? 2. Calculate AH AG and AS for the following reaction given thermodynamic data below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values. HNO,(g) + NH₂(g) → NH.NO,(s) Nitrogen NH₂ (9) NH, (84) HNO, (aq) HNO, (1) HNO.(g) + NH.) → NH.NO ST HNO₂ (9) NH.NO: (S) NH.NO: (aq) AH AG AS AH, (kJ/mol) AG", (kJ/mol) S° (J/mol K) -16.5 192.5 -27.0 111.0 -111.3 146.4 -80.7 155.6 -74.7 266.4 -183.9 151.1 -190.6 259.8 -46.1 -80.0 -207.4 -174.1 -135.1 -365.6 -339.9 3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)? Explain. 4. Based on the signs of AH and AS, in which of the 4 categories does this reaction belong: spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high temperature or spontaneous at low temperature? 5. Use the A Hand AS, calculated in question 2 as well as the equation below to calculate AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results compare to the answers in questions 2 and 4? Be careful with the units, AS was calculated in units of J/(mol*K) while AH was calculated in kl/mol. AG AG @ 298K @ 10K AG @ 10,000K Activate V Go to Setting
Transcribed Image Text:Predict t for the following reaction. Is entropy increasing or decreasing? 2. Calculate AH AG and AS for the following reaction given thermodynamic data below. Pay attention to the phase of matter (s, I. g. aq) when selecting the appropriate values. HNO,(g) + NH₂(g) → NH.NO,(s) Nitrogen NH₂ (9) NH, (84) HNO, (aq) HNO, (1) HNO.(g) + NH.) → NH.NO ST HNO₂ (9) NH.NO: (S) NH.NO: (aq) AH AG AS AH, (kJ/mol) AG", (kJ/mol) S° (J/mol K) -16.5 192.5 -27.0 111.0 -111.3 146.4 -80.7 155.6 -74.7 266.4 -183.9 151.1 -190.6 259.8 -46.1 -80.0 -207.4 -174.1 -135.1 -365.6 -339.9 3. Is the reaction exothermic or endothermic? Is it exergonic or endergonic? Is it spontaneous or nonspontaneous at 298K (note: all thermodynamic data given was determined at 298K)? Explain. 4. Based on the signs of AH and AS, in which of the 4 categories does this reaction belong: spontaneous at all temperature, nonspontaneous at all temperature, spontaneous at high temperature or spontaneous at low temperature? 5. Use the A Hand AS, calculated in question 2 as well as the equation below to calculate AG at 298K (room temp), 10K (low temp), and 10,000K (high temp). How do these results compare to the answers in questions 2 and 4? Be careful with the units, AS was calculated in units of J/(mol*K) while AH was calculated in kl/mol. AG AG @ 298K @ 10K AG @ 10,000K Activate V Go to Setting
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